Question

При разложении 680 г пероксида водорода получено 200 л кислорода(н.у).Вычислите выход продукта реакции от теоретически возможного.ПОМОГИТЕ

Answer 1

2H₂O₂ = 2H₂O + O₂↑
M (H₂O₂) = 2*1 г/моль = 2*16 г/моль = 34 г/моль
n(H₂O₂) = 680 г/ 34 г/моль = 20 моль
n(O₂) = 0,5 n(H₂O₂)
n (O₂) = 0,5 * 20 моль = 10 моль
Vm = 22,4 л/моль (константа)
V (O₂) (теоретический) =  22,4 л/моль * 10 моль = 224 л 
W (выход продукта) = V (практический) / V (теоретический)
W (O₂) = 200 л / 224 л = 0,9 =90 %
Ответ:W(O₂)=90 %

Answer 2

Calculation of Theoretical Yield

To calculate the theoretical yield of a reaction, we need to determine the stoichiometry of the reaction and use it to calculate the amount of product that should be obtained.

In this case, we are given that 680 g of hydrogen peroxide (H2O2) decomposes to produce 200 L of oxygen gas (O2) at standard temperature and pressure (n.u).

The balanced chemical equation for the decomposition of hydrogen peroxide is:

2 H2O2 -> 2 H2O + O2

From the equation, we can see that 2 moles of hydrogen peroxide produce 1 mole of oxygen gas. To calculate the theoretical yield of oxygen gas, we need to convert the given mass of hydrogen peroxide to moles and then use the stoichiometry of the reaction.

The molar mass of hydrogen peroxide (H2O2) is approximately 34 g/mol. Therefore, the number of moles of hydrogen peroxide can be calculated as follows:

moles of H2O2 = mass of H2O2 / molar mass of H2O2 moles of H2O2 = 680 g / 34 g/mol moles of H2O2 = 20 mol

According to the stoichiometry of the reaction, 2 moles of hydrogen peroxide produce 1 mole of oxygen gas. Therefore, the theoretical yield of oxygen gas can be calculated as follows:

moles of O2 = (moles of H2O2 / 2) * 1 moles of O2 = (20 mol / 2) * 1 moles of O2 = 10 mol

Since we are given the volume of oxygen gas at standard temperature and pressure (n.u), we can use the ideal gas law to convert the moles of oxygen gas to liters:

V = n * Vm

where V is the volume, n is the number of moles, and Vm is the molar volume at standard temperature and pressure (22.4 L/mol).

V = 10 mol * 22.4 L/mol V = 224 L

Therefore, the theoretical yield of oxygen gas is 224 L.

Answer

The theoretical yield of oxygen gas obtained from the decomposition of 680 g of hydrogen peroxide is 224 L at standard temperature and pressure (n.u).

Please note that the actual yield of a reaction may be different from the theoretical yield due to various factors such as incomplete reactions, side reactions, and experimental limitations.